Stoichiometry of Solution Reactions

I. VIDEO ON SOLUTION STOICHIOMETRY

II. NOTES ON SOLUTION STOICHIOMETRY

III. EXERCISES ON SOLUTION STOICHIOMETRY

1. Calculate the mass of solid NaCl that must be added to 1.50 L of a 0.100 M AgNO₃ solution to precipitate

all of the Ag⁺ ions in the form of AgCl. Calculate the mass of AgCl formed.

2. Calculate the mass of solid sodium sulfate that must be added to 250.0 mL of a 0.200 M solution of barium

nitrate to precipitate all of the barium ions in the form of barium sulfate. Also calculate the mass of

barium sulfate formed.

3. Calculate the mass of NaI that must be added to 425.0 mL of a 0.100 M Pb(NO₃)₂ solution to precipitate

all of the Pb²⁺ ions as PbI₂. Also calculate the mass of PbI₂ formed.

4. When Ba(NO₃)₂ and K₂CrO₄ react in aqueous solution, the yellow solid BaCrO₄ is formed. Calculate the

mass of BaCrO₄ that forms when 3.50 x 10^-3 mol of solid Ba(NO₃)₂ is dissolved in 265 mL of 0.0100 M

K₂CrO₄ solution.

5. Calculate the mass of the white solid CaCO₃ that forms when 25.0 mL of a 0.100 M Ca(NO₃)₂

solution is mixed with 20.0 mL of a 0.150 M Na₂CO₃ solution.

6. When aqueous solutions of Na₂SO₄ and Pb(NO₃)₂ are mixed, PbSO₄, precipitates. Calculate the mass

of PbSO₄ formed when 1.25 L of 0.0500 M Pb(NO₃)₂ and 2.00 L of 0.0250 M Na₂SO₄ are mixed.

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